The equations representing the combustion of carbon and carbon monoxide are :
`C(s) + O_(2)(g) to CO_(2)(g) DeltaH = -394 (kJ)/(mol)`
`CO(s) + 1/2 O_(2)(g) to CO_(2)(g) DeltaH = -284.5 (kJ)/(mol)`
the heat of formation of 1 mol of CO(g) is :

Options

A. `-109.5 (kJ)/(mol)`
B. `+109.5 (kJ)/(mol)`
C. `+ 180.0 (kJ)/(mol)`
D. `+ 100 (kJ)/(mol)`

Explanation

To find the heat of formation of 1 mole of carbon monoxide (CO), we can use the given combustion reactions of carbon and carbon monoxide. The heat of formation of a compound is defined as the heat change when 1 mole of the compound is formed from its elements in their standard states.

### Step-by-Step Solution:

1. **Write the combustion reactions**:
- The combustion of carbon:
\[
C(s) + O_2(g) \rightarrow CO_2(g) \quad \Delta H = -394 \, \text{kJ/mol}
...